1. Types of Chemical Reactions
Chapter 6

2. 6 Types Synthesis Decomposition Single displacement
Double displacement
Combustion
Neutralization (Chapter 5)

3. Online Resources Animation: http://www.youtube.com/watch?v=tE4668aarck
DEMOS:
Lessons:
(Flintstones)

4. Synthesis
This type of reaction involves the combination of multiple reactants into a single product
Synthesis reactions have a general formula:
F + W ➜ FW

5. Examples 1. Element + Element ➜ Compound
2Al(s) Cl2 (g) ➜ 2 AlCl3 (s)
2. Compound + Element ➜ Compound
PCl3(l) Cl2 (g) ➜ PCl5 (s)
3. Compound + Compound ➜ Compound
SO2(g) H2O(l) ➜ H2SO4(aq)

6. Decomposition
This type of reaction involves the splitting of a single reactant into multiple products
Decomposition reactions have the general formula:
FW ➜ F +W

7. Examples 1. Compound ➜ Element + Element 2HI(g) ➜ H2 (g) + I2 (g)
2. Compound ➜ Compound + Element
2 H2O2(l) ➜ H2O(l) + O2 (g)
3. Compound ➜ Compound + Compound
Ca(OH)2(s) ➜ CaO(s) H2O(l)

8. WORK Read section 6.1 Worksheet
Page 226 to 227, ALL Practice Problems:
Review Questions: Page 229 #1-10

9. Single Displacement
This type of reaction involves an element and a compound as reactants
The element displaces (replaces) one of the elements in the compound
cations replace cations, anions replace anions
Single displacement reactions have the general formula:
FW + B ➜ FB + W

10. Examples Element + Compound  Element + Compound
Zn(s) CuSO4(aq)  Cu (s) ZnSO4(aq)
Mg(s) AgNO3 (aq)  2Ag (s) Mg(NO3)2(aq)
Br2(g) CaI2(aq)  I2 (g) CaBr2(aq)
2 Na(s) H2O(l)  H2 (g) NaOH(aq)
2 Na HOH  H NaOH

11. Double Displacement
This type of reaction involves two compounds as reactants
Positive and negative ions in two compounds appear to “change partners” to form two new compounds with no change in oxidation numbers [ie. Copper (II) stays copper (II)].
Double displacement reactions have the general formula: FW + RB  FB + RW

12. Examples Compound + Compound  Compound + Compound
HCl(aq) NaOH(aq)  NaCl (aq) H2O(l)
2H3PO4 (aq) + 3 Ca(OH)2 (aq)  Ca3(PO4)2 (s) + 6H2O (l)
MnS(s) HCl(aq)  MnCl2 (aq) H2S(g)

13. WORK Read pages 233 to 236 Finish Worksheet
Page 233 to 235, ALL Practice Problems
Review Questions: Page 240 #1-12

14. Combustion
Combustion is a very rapid reaction of a substance with oxygen to produce compounds called oxides.
We often call this process burning.
The following word equation represents a general combustion reaction:
fuel + oxygen  oxides + (energy)

15. Hydrocarbons
Hydrocarbons (compounds with H, C) are the most important fuels that we burn! Gasoline, natural gas (methane), propane, kerosene and matches.
When these burn, the products are mostly CO2 and H2O which are released into the atmosphere. These can contribute to the green house effect.

16. Common Hydrocarbons FORMULA COMMON NAME CHEMICAL NAME CH4 Methane
Carbon tetrahydride
C3H8
Propane
Tricarbon
octahydride
C4H10
Butane
Tetracarbon
decahydride

17. Burning Propane Complete combustion Incomplete combustion
Propane + oxygen  carbon dioxide + water
C3H O  3CO H2O
Incomplete combustion
Propane oxygen  carbon dioxide + water + carbon monoxide + carbon
2C3H O2  2CO2 + 8H2O + 2CO + 2C

18. Complete vs. Incomplete Combustion of Hydrocarbons
Occurs when the right amount of O2 is available to react with the fuel and all the carbon in the fuel is converted into CO2.
The only products are CO2 and H2O.
Incomplete combustion:
This occurs when there is not enough oxygen available to react with the fuel
four products are produced instead of two: CO2, CO, C, H2O
Carbon monoxide is a colourless, odourless, and poisonous gas that can can combine with the haemoglobin in the blood to starve the body of oxygen and cause death!!!
Carbon is the black residue (soot) that you see in fireplaces.

19. Combustion of metals
2 Ca + O2  2 CaO
Combustion & synthesis

20. Combustion of Non-metals
N O2  2 NO2
Combustion & synthesis

21. Homework
Read pages 230 to 232
Page 240 # 9 & 11
Page 242 # 11 & 13

22. Neutralization
A neutralization reaction is a special case of double displacement reaction between an Acid and a Base. The products of a neutralization reaction are always water and a salt (ionic compound).
Examples:
1. HCl(aq) NaOH(aq)  HOH + NaCl
Hydrochloric acid + sodium hydroxide  water + sodium chloride
H2SO4(aq) KOH  2H2O K2SO4
Sulfuric acid + potassium hydroxide  water + potassium sulfate
During a neutralization reaction, the hydrogen ion from the acid reacts with the hydroxide ion from the base
H+ + OH-  H2O

23. Homework
Read Section 5.2
Worksheet